At a certain temperature, Kc for 2 NO(g) + O₂(g) ⇌ 2 NO₂(g) is 1.6 × 10³, and Kc for 2 NO₂(g) ⇌ N₂O₄(g) is 4.0, both with concentrations in mol L⁻¹. What is the value of Kc at this temperature for NO(g) + 1/2 O₂(g) ⇌ 1/2 N₂O₄(g)?

ChemistryMediumHigh School (11–12)Chemical Reactions JEE Main

At a certain temperature, $K_c$ for $2\,\text{NO}(g) + \text{O}_2(g) \rightleftharpoons 2\,\text{NO}_2(g)$ is $1.6 \times 10^{3}$ , and $K_c$ for $2\,\text{NO}_2(g) \rightleftharpoons \text{N}_2\text{O}_4(g)$ is $4.0$ , both with concentrations in $\text{mol L}^{-1}$ . What is the value of $K_c$ at this temperature for $\text{NO}(g) + \tfrac{1}{2}\,\text{O}_2(g) \rightleftharpoons \tfrac{1}{2}\,\text{N}_2\text{O}_4(g)$ ?

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← Nitrosyl bromide breaks down when warmed: 2 NOBr(g) ⇌ 2 NO(g) + Br₂(g). At 350 K, Kc = 1.5 × 10⁻² mol L⁻¹. What is Kp for this reaction at the same temperature, with pressures in bar? Take R = 0.08314 L bar K⁻¹ mol⁻¹.Pyridine, C₅H₅N, is a weak base: C₅H₅N + H₂O ⇌ C₅H₅NH⁺ + OH⁻, with Kb = 1.6 × 10⁻⁹ at 298 K. What is the pH of a 0.25 mol L⁻¹ solution of pyridine at 298 K? Take Kw = 1.0 × 10⁻¹⁴ and log 2 = 0.301. →

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